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Q:
If the number of moles of gas is doubled at constant temperature and volume, the pressure of the gas
A) is halved.
B) is doubled.
C) is quadrupled.
D) remains the same.
Q:
What is the value of the gas constant, R, in units of ?
A) 1.080 10-4
B) 0.1080
C) 62.36
D) 6.236 104
Q:
A balloon filled with helium gas at 20C occupies 2.91 L at 1.00 atm. The balloon is immersed in liquid nitrogen at -196C, raising the pressure to 5.20 atm. What is the volume of the balloon in the liquid nitrogen?
A) 0.15 L
B) 2.1 L
C) 4.0 L
D) 58 L
Q:
The volume of 350. mL of gas at 25C is decreased to 125 mL at constant pressure. What is the final temperature of the gas?
A) -167C
B) 8.9C
C) 70C
D) 561C
Q:
A gas bottle contains 0.650 mol of gas at 730 mm Hg pressure. If the final pressure is 1.15 atm, how many moles of gas were added to the bottle?
A) 0.0680 mol
B) 0.128 mol
C) 0.717 mol
D) 0.778 mol
Q:
A basketball is inflated to a pressure of 1.50 atm in a 20.0C garage. What is the pressure of the basketball outside where the temperature is -5.00C?
A) 1.37 atm
B) 1.42 atm
C) 1.58 atm
D) 1.64 atm
Q:
An "empty" aerosol can at 25C still contains gas at 1.00 atmosphere pressure. If an "empty" can is thrown into a 475C fire, what is the final pressure in the heated can?
A) 5.26 10-2 atm
B) 0.398 atm
C) 2.51 atm
D) 19.0 atm
Q:
"Equal volumes of different gases at the same temperature and pressure contain the same molar amounts" is another way of stating
A) Avogadro's law.
B) Boyle's law.
C) Charles' law.
D) Graham's law.
Q:
An approximation of absolute zero was made from an extrapolation of
A) P vs. 1/V
B) V vs. T
C) n vs. V
D) V vs. 1/T
Q:
Which law does the equation, = k represent?
A) Avogadro's law
B) Boyle's law
C) Charles' law
D) Graham's law
Q:
When temperature-volume measurements are made on 1.0 mol of gas at 1.0 atm, a plot V versus T results in a
A) hyperbola.
B) parabola.
C) sine curve.
D) straight line.
Q:
When pressure-volume measurements are made on 1.0 mol of gas at constant temperature, a plot V versus P results in a
A) hyperbola.
B) parabola.
C) sine curve.
D) straight line.
Q:
Which of the following equations represents "Boyle's law"?
A) = k
B) = k
C) PV = k
D) V = nk
Q:
Which one of the following is not used to describe the condition of a gas?
A) number of moles
B) polarity
C) temperature
D) volume
Q:
A container filled with gas is connected to an open-end U-tube manometer that is filled with mineral oil. The pressure in the gas container is 773 mm Hg and atmospheric pressure is 754 mm Hg. What will be the difference in the levels of mineral oil in the two arms of the manometer if the densities of Hg and mineral oil are 13.6 g/mL and 0.822 g/mL respectively?
A) 1.15 mm
B) 15.6 mm
C) 19.0 mm
D) 314 mm
Q:
If the pressure in a gas container that is connected to an open-end U-tube manometer is 106 kPa and the pressure of the atmosphere at the open end of the tube is 742 mm Hg, the level of mercury in the tube will be
A) 53 mm higher in the arm open to the atmosphere.
B) 53 mm higher in the arm connected to the gas cylinder.
C) 636 mm higher in the arm open to the atmosphere.
D) 636 mm higher in the arm connected to the gas cylinder.
Q:
What is the pressure in a gas container that is connected to an open-end U-tube manometer if the pressure of the atmosphere is 752 torr and the level of mercury in the arm connected to the container is 8.60 cm higher than the level of mercury open to the atmosphere?
A) 666 mm Hg
B) 743 mm Hg
C) 761 mm Hg
D) 838 mm Hg
Q:
In an open end manometer, one end of a U-tube filled with mercury is attached to a gas-filled container and the other end is open to the atmosphere. If the gas pressure in the container is less than atmospheric pressure
A) Hg will be forced out of the open end of the U-tube.
B) the difference between the Hg levels in the two arms will be greater than 76 cm.
C) the Hg level will be higher in the arm connected to the container.
D) the Hg level will be higher in the arm open to the atmosphere.
Q:
Suppose you needed to closely monitor small changes in pressure inside a container using an open end manometer. For the best accuracy, the substance in the manometer should
A) be a solid.
B) be mercury.
C) have a high density.
D) have a low density.
Q:
If mercury (density = 13.6 g/cm3) at a height of 745 mm Hg in a mercury barometer is replaced with water (density = 1.00 g/cm3), under the same conditions the height of water will be
A) 0.180 ft
B) 2.44 ft
C) 33.2 ft
D) 399 ft
Q:
The pressure in the eye of a hurricane is less than atmospheric pressure. Which one of the following pressure readings could not have been taken in the eye of a hurricane?
A) 15 lbs/in2
B) 69 cm Hg
C) 690 mm Hg
D) 9.22 104 Pa
Q:
Automobile tires are typically inflated to about 30 pounds of pressure per square inch. What is the typical air pressure of a tire in kPa?
A) 2.0 10-3 kPa
B) 2.0 kPa
C) 2.1 102 kPa
D) 2.1 105 kPa
Q:
Which is the smallest quantity of pressure?
A) 1 atm
B) 1 centimeter of Hg
C) 1 mm Hg
D) 1 pascal
Q:
Which of the following is not equivalent to 1 atm pressure?
A) 10 cm Hg
B) 14.7 lb/in2
C) 101 kPa
D) 760 mm Hg
Q:
The SI unit for pressure is the
A) atmosphere.
B) MM Hg.
C) newton.
D) pascal.
Q:
Pressure is defined as
A) force divided by unit area.
B) force times unit area.
C) mass divided by acceleration.
D) mass times acceleration.
Q:
Which of the following instruments directly measures the pressure of a gas?
A) spectrometer
B) manometer
C) polarimeter
D) gas chromatograph
Q:
Carbon dioxide is a gas which causes environmental concern because of the greenhouse effect. What is the approximate percentage (by volume) of CO2 in the atmosphere?
A) less than 0.1%
B) about 1%
C) about 10%
D) more than 20%
Q:
What are the signs of H, S, and G for the following spontaneous change?A) H = +, S = +, G = -B) H = +, S = -,G = -C) H = -, S = +, G = -D) H = -, S = -, G = -
Q:
What are the signs of H, S, and G for the following spontaneous change?A) H = +, S = +, G = -B) H = +, S = -, G = -C) H = -, S = +, G = -D) H = -, S = -, G = -
Q:
What are the signs of H, S, and G for the following spontaneous change?A) H = +, S = +, G = -B) H = +, S = -, G = -C) H = -, S = +, G = -D) H = -, S = -, G = -
Q:
The intermediate, T, + S is represented by
A) arrow C.
B) line D.
C) line E.
D) line F.
Q:
The product, Z, is represented by
A) arrow A.
B) line D.
C) line E.
D) line F.
Q:
The reactants, R + 2 S, are represented by
A) arrow B.
B) line D.
C) line E.
D) line F.
Q:
The net reaction is represented by
A) arrow A.
B) arrow B.
C) arrow C.
D) line F.
Q:
Step (2) in the reaction is represented by
A) arrow A.
B) arrow B.
C) arrow C.
D) line E.
Q:
Step (1) in the reaction is represented by
A) arrow A.
B) arrow B.
C) arrow C.
D) line E.
Q:
Imagine a reaction that results in a change in both volume and temperature, as shown in the diagram below. What is the sign of the work being done, and what is the sign of the enthalpy change involved in this reaction?A) w = + and H = +B) w = + and H = -C) w = - and H = +D) w = - and H = -
Q:
Imagine a reaction that results in a change in both volume and temperature, as shown in the diagram below. What is the sign of the work being done and the sign of the enthalpy change involved in this reaction?A) w = + and H = +B) w = + and H = -C) w = - and H = +D) w = - and H = -
Q:
Imagine a reaction that results in a change in both volume and temperature, as shown in the diagram below. What is the sign of the work being done, and what is the sign of the enthalpy change involved in this reaction?A) w = + and H = +B) w = + and H = -C) w = - and H = +D) w = - and H = -
Q:
Imagine a reaction that results in a change in both volume and temperature, as shown in the diagram below. What is the sign of the work being done and the sign of the enthalpy change involved in this reaction?A) w = + and H = +B) w = + and H = -C) w = - and H = +D) w = - and H = -
Q:
The enthalpy of fusion of naphthalene, C10H8, is 19.1 kJ/mol at 78.2C, its melting point. Calculate the entropy of fusion at the melting point.A) Sfus = 244 J/(K mol)B) Sfus = 54.4 J/(K mol)C) Sfus = 1.49 J/(K mol)D) Sfus = -1.49 J/(K mol)
Q:
Calculate G for the reaction below and tell whether it is spontaneous or nonspontaneous under standard conditions at 25C.2 S (s) + 3 O2 (g) + 2 H2O (l) -> 2 H2SO4 (l) H = -1056 kJ/molS= -505 J/molA) G = -1207 kJ and the process is spontaneous.B) G = -1207 kJ and the process is nonspontaneous.C) G = -906 kJ and the process is spontaneous.D) G = -906 kJ and the process is nonspontaneous.
Q:
For the conversion of water to ice at 25C and 1 atm,A) G is negative and H is negative.B) G is negative and H is positive.C) G is positive and H is negative.D)G is positive and H is positive.
Q:
For the conversion of ice to water at 0C and 1 atm,A) G is zero, H is positive, and S is negative.B) G is zero, H is positive, and S is positive.C) G is negative, H is negative, and S is positive.D) G is positive, H is negative, and S is positive.
Q:
He gas is contained in a one-liter flask that is connected to an empty one-liter flask with a closed stopcock between the two flasks. When the stopcock is opened some of the He enters the evacuated flask. For this systemA) H is negative and S is positiveB) H is zero and S is positiveC) H is zero and S is negativeD) H is positive and S is negative
Q:
Methanol can be produced from carbon monoxide and hydrogen with suitable catalysts:CO(g) + 2 H2(g) -> CH3OH(l) at 25C H = -128.1 kJ and S = -332 J/KFind G at 25C.A) -157.2 kJB) -29.1 kJC) 98.9 kJD) 157.2 kJ
Q:
When heated, mercury(II) oxide decomposes into elemental mercury and oxygen:2 HgO(s) -> 2 Hg(l) + O2(g) H = 181.6 kJ S = 216.4 J/KEstimate the temperature at which HgO should begin to decompose if the partial pressure of O2(g) is constant at 1.00 atm.A) -34.8CB) 34.8CC) 566CD) 840C
Q:
Consider the conversion of white tin to gray tin:Sn(white) -> Sn(gray) H = -2.09 kJ S = -7.41 J/KBased on these data,A) white tin is stable below 9C and gray tin is stable above 9C.B) gray tin is stable below 9C and white tin is stable above 9C.C) white tin is stable below 15C and gray tin is stable above 15C.D) gray tin is stable below 15C and white tin is stable above 15C.
Q:
If a reaction with a negative value of S is nonspontaneous at constant temperature and pressure,A) G is negative and H may be positive or negative.B) G is negative and H is positive.C) G is positive and H may be positive or negative.D) G is positive and H is positive.
Q:
If an endothermic reaction is spontaneous at constant temperature and pressure,A) G is negative and S may be positive or negative.B) G is negative and S is positive.C) G is positive and S is negative.D) G is positive and S may be positive or negative.
Q:
What is the thermodynamic criterion for equilibrium for a reaction at constant temperature and pressure (PV work only)?A) S = 0B) G = 0C) S > 0D) G < 0
Q:
The reaction 4 Ag(s) + O2(g) -> 2 Ag2O(s) favors Ag2O at low temperature, but it favors Ag and O2 at high temperatures. How can this be explained in terms of H and S?A) H is negative and S is negative.B) H is negative and S is positive.C) H is positive and S is negative.D) H is positive and S is positive.
Q:
Which combination always results in a reaction being spontaneous?A) H is negative and S is negative.B) H is negative and S is positive.C) H is positive and S is negative.D) H is positive and S is positive.
Q:
Which is not a spontaneous process?
A) combustion of gasoline to produce carbon dioxide and water
B) diffusion of perfume in a room
C) dissolution of sodium chloride in water
D) freezing of water at 1C
Q:
Determine the sign of S for each of the following:I. The mixing of two gases at a given temperature and pressureII. C(s) + 2 H2O(g) -> CO2(g) + 2 H2(g)A) S is negative for I and negative for II.B) S is negative for I and positive for II.C) S is positive for I and negative for II.D) S is positive for I and positive for II.
Q:
Which of the following is not true?
A) A spontaneous reaction need not occur immediately.
B) A spontaneous reaction must be exothermic and must have an increase in entropy.
C) The reverse of a nonspontaneous reaction is always spontaneous.
D) A spontaneous reaction is one that can proceed on its own.
Q:
For the of freezing liquid ethanol at a given temperature and pressure,A) H is negative and S is negative.B) H is negative and S is positive.C) H is positive and S is negative.D) H is positive and S is positive.
Q:
For the expansion of an ideal gas into a vacuum at constant temperature, H = 0. What can be said about E and S?A) E is negative and S is positive.B) E is zero and S is positive.C) E is negative and S is zero.D) E is positive and S is negative.
Q:
Which thermodynamic function is most related to disorder and probability?
A) enthalpy
B) internal energy
C) entropy
D) heat capacity
Q:
Determine the sign of ΔS for each of the following:I. C6H6(s) -> C6H6(l)II. 2 SO2(g) + O2(g) -> 2 SO3(g)A) S should be negative for I and negative for II.B) S should be negative for I and positive for II.C) S should be positive for I and negative for II.D) S should be positive for I and positive for II.
Q:
For the reaction, NH3(g) -> N(g) + 3 H(g), one would expectA) H to be negative and S to be negative.B) H to be negative and S to be positive.C) H to be positive and S to be negative.D) H to be positive and S to be positive.
Q:
At a given temperature and pressure, which of the following would be expected to have the greatest molar entropy?
A) Br2(s)
B) Br2(l)
C) Br2(g)
D) All of these would be expected to have the same molar entropy.
Q:
Which of the following can be interpreted as a measure of randomness?
A) enthalpy
B) entropy
C) free energy
D) temperature
Q:
Which of CH4(g), C2H2(g), and CH3OH(l) provides the most energy per gram upon combustion and which provides the least?CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(l) H = -890 kJ2 C2H2(g) + 5 O2(g) -> 4 CO2(g) + 2 H2O(l) H = -2599 kJ2 CH3OH(l) + 3 O2(g) -> 2 CO2(g) + 4 H2O(l) H = -1453 kJA) C2H2 provides the most energy per gram and CH4 the least.B) C2H2 provides the most energy per gram and CH3OH the least.C) CH4 provides the most energy per gram and CH3OH the least.D) CH4 provides the most energy per gram and C2H2 the least.
Q:
The heat of combustion per mole for acetylene, C2H2(g), is -1299.5 kJ/mol. Assuming that the combustion products are CO2(g) and H2O(l), and given that the enthalpy of formation is -393.5 kJ/mol for CO2(g) and -285.8 kJ/mol for H2O(l), find the enthalpy of formation of C2H2(g).
A) -846.1 kJ/mol
B) -620.2 kJ/mol
C) -226.7 kJ/mol
D) +226.7 kJ/mol
Q:
Calculate the enthalpy of combustion per mole for C6H12O6. Assume that the combustion products are CO2(g) and H2O(l). A) -5336 kJ/mol
B) -2816 kJ/mol
C) -1939 kJ/mol
D) 580.7 kJ/mol
Q:
Given that H= -311 kJ for the hydrogenation of acetylene, C2H2:H C H(g) + 2 H2(g) ->CH3-CH3(g)and the following bond dissociation energies, estimate a value for the C-to-C triple bond dissociation energy.A) 1050 kJ/molB) 833 kJ/molC) 807 kJ/molD) 397 kJ/mol
Q:
Use the given average bond dissociation energies, D, to estimate H for the reaction of methane, CH4(g), with fluorine according to the equation:CH4(g) + 2 F2(g) -> CF4(g) + 2 H2(g)A) -716 kJB) -318 kJC) +318 kJD) +716 kJ
Q:
One method for making ethanol, C2H5OH, involves the gas-phase hydration of ethylene, C2H4:Estimate H for this reaction from the given average bond dissociation energies, D.A) -580 kJB) -35 kJC) +35 kJD) 580 kJ
Q:
Which is expected to have the largest carbon-oxygen bond dissociation energy?A) COB) CO2C) HCO2HD) CO32-
Q:
For which reaction is H expected to be most positive?A) N2(g) -> 2 N(g)B) O2(g) ->2 O(g)C) 2 N(g) -> N2(g)D) 2 O(g) -> O2(g)
Q:
For the reaction 2CH4 (g) + 3 Cl2 (g) -> 2 CHCl3 (l) + 3 H2 (g), H = -118.6 kJ.Hf = -134.1 kJ/mol for CHCl3 (l). Find Hf for CH4 (g).A) -193.4 kJ/molB) -74.8 kJ/molC) 74.8 kJ/molD) 193.4 kJ/mol
Q:
Acetylene torches utilize the following reaction:2 C2H2(g) + 5 O2(g) ->4 CO2(g) + 2 H2O(g)Use the given standard enthalpies of formation to calculate H for this reaction.A) 2512.4 kJB) 1256.2 kJC) -1256.2 kJD) -2512.4 kJ
Q:
Ethyl alcohol is produced by the fermentation of glucose, C6H12O6.C6H12O6(s) -> 2 C2H5OH(l) + 2 CO2(g) H = -69.1 kJGiven that the enthalpy of formation is -277.7 kJ/mol for C2H5OH(l) and -393.5 kJ/mol for CO2(g), find the enthalpy of formation for C6H12O6.A) -1411.5 kJ/molB) -1273.3 kJ/molC) -740.3 kJ/molD) -602.1 kJ/mol
Q:
Use the given standard enthalpies of formation to calculate H for the following reaction3 Fe2O3(s) + CO(g) -> 2 Fe3O4(s) + CO2(g).A) -5213.4 kJB) -577.2 kJC) -47.2 kJD) +47.2 kJ
Q:
Which equation represents the reaction whose H, represents the standard enthalpy of formation of CHCl3(l) at 25C? (i.e., for which is H = Hf of CHCl3)A) CHCl3(l) -> C(s) + H(g) + 3 Cl(g)B) C(s) + H(g) + 3 Cl(g) -> CHCl3(l)C) C(s) + 1/2 H2(g) + 3/2 Cl2(g) -> CHCl3(l)D) 2 C(s) + H2(g) + 3 Cl2(g) -> 2 CHCl3(l)
Q:
The values of Hf for the three states of benzene are approximately -22 kcal/mol, -11 kcal/mol, and 20 kcal/mol. Which is the value for solid benzene?A) -22 kcal/molB) -11 kcal/molC) 20 kcal/molD) cannot be determined without additional information
Q:
Which is expected to have the most negative standard enthalpy of formation?
A) H2(g)
B) O2(g)
C) H2O(g)
D) H2O(l)
Q:
For which should the standard heat of formation Hf, be zero at 25C?A) O(g)B) O2(g)C) O3(g)D) all the above